Solid state forms of a quinazoline derivative and its use as a braf inhibitor

ABSTRACT

This application relates to various salts and solid state forms of Compound (I). This application also relates to pharmaceutical compositions and therapeutic uses of these materials and compositions.

BACKGROUND OF THE INVENTION Field of the Invention

This application relates to various salts of the following compound (hereinafter referred to as Compound I)

as well as solid state forms of Compound I and its salts and pharmaceutical compositions comprising the same. This application also relates to therapeutic uses of these materials and compositions.

SUMMARY OF THE INVENTION

BRAF is a member of the RAF kinase family of serine/threonine-specific protein kinases. The protein plays a role in regulating the MEK/ERK signaling pathway, which effects cell division, differentiation, and secretion. Acquired mutations in the BRAF gene (i.e., oncogene) in adults can constituently activate the kinases MEK and ERK, thereby fueling cancer growth. Several mutated forms of BRAF have been identified in cancers including melanoma, colorectal cancers, papillary thyroid carcinomas, low-grade serous ovarian cancers, and non-small cell lung cancers. The V600E mutation, which is found in the majority of cases (˜80%) in these types of cancers and in over 50% of patients with melanoma, is an activating mutation resulting in approximately 500-fold greater activity relative to wild type (wt) BRAF (Curtin et al 2005, Davies et al 2002). The increase in kinase activity causes hyperstimulation of downstream signaling pathways, which can impart immortalization of and tumorigenic potential to cells. Not only is BRAF^(V600E) oncogenic, but recent evidence also indicates that this genotype contributes to the development of benign lesions in various tissues, and can progress to a full malignant phenotype in the context of additional genetic events (Michaloglou et al 2008).

Inhibition of the BRAF^(V600E) protein has been shown in animals and in humans to have a profound effect on tumor growth. Results from clinical studies in patients with the BRAF^(V600E) mutation have shown clinically significant and statistically significant superior survival, progression-free survival, and tumor response compared with previous standard therapies. For example, vemurafenib is a BRAF^(V600E) inhibitor that is approved in the United States for patients with unresectable or metastatic melanoma with the BRAF^(V600E) mutation. Approximately half of patients who received vemurafenib responded favorably, with longer progression-free survival and a significant reduction in the risk of death as compared to other available therapies (Chapman et al 2011).

Various BRAF inhibitors have been reported. For example, WO 2009/117080 discloses quinazoline derivatives as modulators of RAF kinase, including BRAF kinase. Compound I has the following structure:

and the following chemical names: 1-[3-(6,7-dimethoxy-quinazolin-4-yloxy)-phenyl]-3-[5-(2,2,2-trifluoro-1,1-dimethyl-ethyl)-isoxazol-3-yl]-urea or N-[3-[(6,7-dimethyoxy-4-quinazolinyl)oxy]phenyl]-N′-[5-(2,2,2-trifluoro-1,1-dimethylethyl)-3-isoxazolyl]urea. Compound I is a potent and selective inhibitor of BRAF kinase including mutated versions. For example, Compound I inhibits BRAF V600E at low nanomolar concentrations in vitro in intact cells as well as in isolated systems.

Different salt and/or solid state forms of Compound I can have significantly different physical properties, which either alone or in combination, can affect bioavailability. Similarly, the physical properties of the various salt/solid state forms of Compound I can also affect other aspects such as processing and storage characteristics. All of these properties are factors in selecting a salt and/or solid state form for clinical testing and commercial development.

A number of different salt forms of Compound I have been identified and are described herein. Various solid state forms of these salts as well as the solid state form of the free base of Compound I were also identified. The preparation and physical characterization of these materials are also provided herein.

The present application also provides pharmaceutical compositions comprising Compound I (free base) and/or salts of Compound I which may be used for treating various disease states such as melanoma, colorectal cancer, papillary thyroid carcinoma, low-grade serous ovarian cancer, and non-small cell lung cancer. In another aspect the present application provides pharmaceutical compositions comprising Compound I (free base) and/or salts of Compound I for treating a disease state associated with a mutated form of BRAF kinase.

BRIEF DESCRIPTION OF THE DRAWINGS

FIG. 1 illustrates the XRPD pattern of Form A_(o).

FIG. 2 illustrates the variable temperature XRPD patterns of Form A_(o) (25° C.-225° C.).

FIG. 3 illustrates the overlay of DSC and TGA curves of Form A_(o).

FIG. 4 illustrates the gravimetric vapor sorption isotherm of Form A_(o).

FIG. 5 illustrates the XRPD patterns of Form A_(o) before and after GVS analysis.

FIG. 6 illustrates the infrared spectra of Form A_(o).

FIG. 7 is a photograph of Form A_(o) at room temperature.

FIG. 8 illustrates the XRPD pattern of bromide Form A₁.

FIG. 9 illustrates the overlay of DSC and TGA curves of bromide Form A₁.

FIG. 10 illustrates the GVS isotherm of bromide Form A₁.

FIG. 11 illustrates the kinetic data/mass plot of bromide Form A₁.

FIG. 12 illustrates the XRPD patterns of bromide Form A₁ before and after GVS analysis.

FIG. 13 illustrates the FTIR spectra of bromide Form A₁.

FIG. 14 is a photograph of bromide Form A₁ at room temperature.

FIG. 15 illustrates the XRPD pattern of chloride Form A₁.

FIG. 16 illustrates the variable temperature XRPD patterns of chloride Form A₁ (25° C.-245° C.).

FIG. 17 illustrates the overlay of DSC and TGA curves of chloride Form A₁.

FIG. 18 illustrates the GVS isotherm of chloride Form A₁.

FIG. 19 illustrates the XRPD patterns of chloride Form A₁ before and after GVS analysis.

FIG. 20 illustrates the FTIR spectrum of chloride Form A₁.

FIG. 21 is a photograph of chloride Form A₁ at room temperature.

FIG. 22 illustrates the XRPD pattern of malonate Form A₁.

FIG. 23A illustrates the overlay of DSC and TGA curves of malonate Form A₁.

FIG. 23B illustrates the GVS isotherm of malonate Form A₁

FIG. 23C illustrates a kinetic data/mass plot of malonate Form A₁

FIG. 24 illustrates the FTIR spectrum of malonate Form A₁.

FIG. 25 is a photograph of malonate Form A₁ at room temperature.

FIG. 26 illustrates the XRPD pattern of phosphate Form A₁.

FIG. 27 illustrates the overlay of DSC and TGA curves of phosphate Form A₁.

FIG. 28 illustrates the GVS isotherm of phosphate Form A₁.

FIG. 29 illustrates the kinetic data/mass plot of phosphate Form A₁.

FIG. 30 illustrates the XRPD patterns of phosphate Form A₁ before and after GVS analysis.

FIG. 31 illustrates the FTIR Spectrum of phosphate Form A₁.

FIG. 32 is a photograph of phosphate Form A₁ at room temperature.

DETAILED DESCRIPTION OF THE PREFERRED EMBODIMENT

Pharmaceutical solids (also referred to as active pharmaceutical ingredients or APIs) can exist m more than one solid state form (i.e., crystalline, noncrystalline/amorphous, quasicrystalline/organized aggregate). Polymorphism is defined as the ability of a solid compound to exist in more than one crystalline form with the same covalent chemical structure, but different supra-molecular structures and ordered arrangements of molecules within the crystalline lattice. In addition to exhibiting polymorphism, many pharmaceutical solids form hydrates and organic solvates, which themselves can be crystalline and exhibit polymorphism. Hydrates can be stoichiometric or non-stoichiometric. In a stoichiometric hydrate, the water molecules are (relatively) tightly associated with or bound to the pharmaceutical compound as well as to other water molecules and as a result are integral to the crystal lattice. In contrast, the water molecules of a non-stoichiometric hydrate (sometimes referred to as a variable hydrate) are more loosely associated with the pharmaceutical compound and the crystal lattice.

It is well recognized that different solid state forms of the same compound can exhibit significantly different chemical and physical properties including color, morphology, stability, solubility, dissolution and bioavailability. As with all pharmaceutical compounds and compositions, the chemical and physical properties of a particular solid state form of a compound are important to its commercial development. These properties include, but are not limited to: (1) packing properties such as molar volume, density and hygroscopicity, (2) thermodynamic properties such as melting temperature, vapor pressure and solubility, (3) kinetic properties such as dissolution rate and stability (including chemical and solid state stability at ambient conditions, especially to moisture, and under storage conditions including accelerated storage conditions, i.e., high relative humidity and temperature), (4) surface properties such as surface area, wettability, interfacial tension and shape, (5) mechanical properties such as hardness, tensile strength, compactibility, handling, flow and blend; and (6) filtration properties. These properties can affect, for example, processing and storage of pharmaceutical compositions, sometimes referred to as drug product and/or of the processing and storage of an API, which is sometimes referred to as drug substance. As mentioned above, different solid state forms of the API can have different rates of solubility which can translate into differences in bioavailability in vivo.

In general, the solid state form of a compound (or salt of that compound) can be distinguished from another solid state form of the same compound (or salt) using one or more of the following techniques: x-ray powder diffraction (XRPD), thermal techniques including thermogravimetric analysis (TGA) and differential scanning calorimetry (DSC), Gravimetric Vapor Sorption (GVS), as well as Infrared (IR), Raman and/or solid state NMR (ssNMR) spectroscopy. In particular XRPD is particularly useful in identifying and/or distinguishing between polymorphs of a given compound (or salt of that compound) because it is generally accepted and understood that every crystalline phase of a given compound (or salt of that compound) produces a characteristic x-ray diffraction pattern. See generally, USP 35, <941> pp 427-431 (Dec. 1, 2012). It is also generally accepted that complementary analytical techniques can be used to confirm the identity of a particular crystalline form.

Table 1 sets forth the salts described in this application.

TABLE 1 Salts Of Compound I Salt Form Solid State Description Bromide A₁ Crystalline anhydrate Chloride A₁ Crystalline anhydrate Malonate A₁ Crystalline anhydrate Phosphate A₁ Crystalline anhydrate

The solid state descriptions in Table 1 were assigned primarily based upon XRPD pattern. The subscript “1” after the letter “A” was assigned to indicate the mono-salt form. As used herein, the subscript “O” is used to denote a free base (non-salt) form. One of skill in the art would readily understand that descriptors, such as, for example “the chloride salt” or “chloride-Compound I salt” or “Compound I-chloride salt”, refer to the HCl (or hydrochloride) salt of Compound I.

The term “isolating” as used herein, means separating a compound from a solvent, anti-solvent, or a mixture of solvent and anti-solvent to provide a solid, semisolid or syrup. This is typically accomplished by means such as centrifugation, filtration with or without vacuum, filtration under positive pressure, distillation, evaporation or a combination thereof. Isolating may or may not be accompanied by purifying during which the chemical, chiral or chemical and chiral purity of the isolate is increased. Purifying is typically conducted by means such as crystallization, distillation, extraction, filtration through acidic, basic or neutral alumina, filtration through acidic, basic or neutral charcoal, column chromatography on a column packed with a chiral stationary phase, filtration through a porous paper, plastic or glass barrier, column chromatography on silica gel, ion exchange chromatography, recrystallization, normal-phase high performance liquid chromatography, reverse-phase high performance liquid chromatography, trituration and the like.

The term “polymorphic” or “polymorphism” is defined as the possibility of at least two different crystalline arrangements for the same chemical molecule.

The term “solid state form” as used herein, refers to both crystalline and amorphous (non-crystalline) forms of Compound I and mixtures thereof in any ratio. It should be understood that the term solid state form includes crystalline and amorphous (non-crystalline) hydrates and solvates of Compound I as well.

The term “chemical form” as used herein, refers to a salt or non-salt (free base) forms of Compound I or mixtures thereof in any ratio. It should be understood that the term chemical form includes hydrates and solvates of Compound I as well as hydrates and solvates of salts of Compound I as well.

The term “solute” as used herein, refers to a substance dissolved m another substance, usually the component of a solution present in the lesser amount.

The term “solution,” as used herein, refers to a mixture containing at least one solvent and at least one compound at least partially dissolved in the solvent.

The term “solvate,” as used herein, refers to a crystalline material that contains solvent molecules within the crystal structure.

The term “solvent,” as used herein, means a substance, typically a liquid, that is capable of completely or partially dissolving another substance, typically a solid. Unless otherwise specified, typical solvents for the practice of this invention include, but are not limited to, water, acetic acid, acetone, acetonitrile, 1-butanol, 2-butanol, 2-butanone, butyronitrile, tert-butanol, chlorobenzene, chloroform, cyclohexane, 1,2-dichloloroethane, dichloromethane, diethylene glycol dibutyl ether, diisopropyl amine, diisopropyl ether, 1,2-dimethoxyethane, N,N-dimethylacetamide, N,N-dimethylformamide, dimethyl sulfoxide, 1,4-dioxane, ethyleneglycoldiemethylether, ethanol, ethyl acetate, ethylene glycol, ethyl formate, formic acid, heptane, isobutyl alcohol, isopropyl acetate, isopropyl amme, methanol, methoxy benzene, methyl acetate, methyl isobutyl ketone, 2-methyltetrahydrofuran, methyl tert-butyl ether, 1:1 formamide:water, 1:1 N-methylpyrrolidinone, 2-pentanone, 3-pentanone, 1 pentanol, 1,2-propanediol, 2-propanol, 1-propanol, propanonitrile, pyridine, tetrahydrofuran, tetrahydropyran, toluene, triethyl amine, xylene, mixtures thereof and the like.

The term “therapeutically effective amount,” as used herein, refers to the amount determined to be required to produce the physiological effect intended and associated with a given drug, as measured according to established pharmacokinetic methods and techniques, for the given administration route. Appropriate and specific therapeutically effective amounts can be readily determined by the attending diagnostician, as one skilled in the art, by the use of conventional techniques. A therapeutically effective amount or dose will vary depending upon a number of factors, including the type and extent of progression of the disease or disorder, the overall health status of the particular patient, the relative biological efficacy of the compound selected, the formulation of the active agent with appropriate excipients, and the route of administration. Typically, the solid state and chemical forms of the invention would be administered at lower dosage levels, with a gradual increase in dose until the desired effect is achieved.

Unless stated otherwise, percentages stated throughout this specification are weight/weight (w/w) percentages.

The term “pharmaceutically acceptable excipients,” as used herein, includes any and all solvents, dispersion media, coatings, antibacterial and antifungal agents, isotonic and absorption delaying agents and the like. The use of such media and agents for pharmaceutical active substances is well known in the art, such as in Remington: The Science and Practice of Pharmacy, 20th ed.; Gennaro, A. R., Ed.; Lippincott Williams & Wilkins: Philadelphia, Pa., 2000. Except insofar as any conventional media or agent is incompatible with the active ingredient, its use in the therapeutic compositions is contemplated. Supplementary active ingredients can also be incorporated into the compositions.

For therapeutic purposes, the crystalline or amorphous forms of the present invention can be administered by any means that results in the contact of the active agent with the agent's site of action in the body of the subject. The solid state forms of Compound I and/or its salts may be administered by any conventional means available for use in conjunction with pharmaceuticals, either as individual therapeutic agents or in combination with other therapeutic agents, such as, for example, analgesics. The solid and chemical forms of the present invention are preferably administered in therapeutically effective amounts for the treatment of the diseases and disorders described herein to a subject that has been determined to be in need of such treatment.

Typical dose ranges are from about 0.01 mg/kg to about 500 mg/kg of body weight per day. A preferred unit dose for an adult human includes about 25, 50, 100 and 200 mg of the selected solid state form or chemical form of Compound I, which may be administered one to four times a day. In an alternate method of describing a therapeutically effective dose, is a particular dose that is necessary to achieve a particular blood serum level.

The solid state and/or chemical forms of the present invention may be formulated into pharmaceutical compositions by admixture with one or more pharmaceutically acceptable excipients. The excipients are selected on the basis of the chosen route of administration and standard pharmaceutical practice, as described, for example, in Remington: The Science and Practice of Pharmacy, 20th ed.; Gennaro, A. R., Ed.; Lippincott Williams & Wilkins: Philadelphia, Pa., 2000. The compositions may be formulated to control and/or delay the release of the active agent(s), as in fast-dissolve, modified-release, or sustained-release formulations. Such controlled-release, or extended release compositions may utilize, for example biocompatible, biodegradable lactide polymers, lactide/glycolide copolymers, polyoxyethylene-polyoxypropylene copolymers, or other solid or semisolid polymeric matrices known in the art.

The compositions of the present invention can be prepared for administration by oral means; parenteral means, including intravenous, intramuscular, and subcutaneous routes; topical or transdermal means; transmucosal means, including rectal, vaginal, sublingual and buccal routes; ophthalmic means; or inhalation means. Preferably the compositions are prepared for oral administration, particularly in the form of tablets, capsules or syrups; for parenteral administration, particularly in the form of liquid solutions, suspensions or emulsions; for intranasal administration, particularly in the form of powders, nasal drops, or aerosols; or for topical administration, such as creams, ointments, solutions, suspensions aerosols, powders and the like.

For oral administration, the tablets, pills, powders, capsules, troches and the like can contain one or more of the following: diluents or fillers such as starch, or cellulose; binders such as microcrystalline cellulose, gelatins, or polyvinylpyrrolidones; disintegrants such as starch or cellulose derivatives; lubricants such as talc or magnesium stearate; glidants such as colloidal silicon dioxide; sweetening agents such as sucrose or saccharin; or flavoring agents such as peppermint or cherry flavoring. Capsules may contain any of the aforementioned excipients, and may additionally contain a semi-solid or liquid carrier, such as a polyethylene glycol. The solid oral dosage forms may have coatings of sugar, shellac, or enteric agents. Liquid preparations may be in the form of aqueous or oily suspensions, solutions, emulsions, syrups, elixirs, etc., or may be presented as a dry product for reconstitution with water or other suitable vehicle before use. Such liquid preparations may contain conventional additives such as surfactants, suspending agents, emulsifying agents, diluents, sweetening and flavoring agents, dyes and preservatives.

The compositions may also be administered parenterally. The pharmaceutical forms acceptable for injectable use include, for example, sterile aqueous solutions, or suspensions. Aqueous carriers include mixtures of alcohols and water, buffered media, and the like. Non-aqueous solvents include alcohols and glycols, such as ethanol, and polyethylene glycols; oils, such as vegetable oils; fatty acids and fatty acid esters, and the like. Other components can be added including surfactants; such as hydroxypropylcellulose; isotonic agents, such as sodium chloride; fluid and nutrient replenishers; electrolyte replenishers; agents which control the release of the active compounds, such as aluminum monostearate, and various co-polymers; antibacterial agents, such as chlorobutanol, or phenol; buffers, and the like. The parenteral preparations can be enclosed in ampules, disposable syringes or multiple dose vials. Other potentially useful parenteral delivery systems for the active compounds include ethylene-vinyl acetate copolymer particles, osmotic pumps, implantable infusion systems, and liposomes.

Other possible modes of administration include formulations for inhalation, which include such means as dry powder, aerosol, or drops. They may be aqueous solutions containing, for example, polyoxyethylene-9-lauryl ether, glycocholate and deoxycholate, or oily solutions for administration in the form of nasal drops, or as a gel to be applied intranasally. Formulations for topical use are in the form of an ointment, cream, or gel. Typically these forms include a carrier, such as petrolatum, lanolin, stearyl alcohol, polyethylene glycols, or their combinations, and either an emulsifying agent, such as sodium lauryl sulfate, or a gelling agent, such as tragacanth. Formulations suitable for transdermal administration can be presented as discrete patches, as in a reservoir or microreservoir system, adhesive diffusion-controlled system or a matrix dispersion-type system. Formulations for buccal administration include, for example lozenges or pastilles and may also include a flavored base, such as sucrose or acacia, and other excipients such as glycocholate. Formulations suitable for rectal administration are preferably presented as unit-dose suppositories, with a solid based carrier, such as cocoa butter, and may include a salicyclate.

Solvents and Acids

The pK_(a) values of Compound I were calculated by ACD Software, version 101. The pK_(a) of 2.8 for the quinazoline moiety suggests that for salt screening may be attempted with a wide range of acids. This does not, however, guarantee or predict success for all conditions or for all acids that were selected for testing. Salt or co-crystal formation was attempted with the 24 acids listed in Table 2. These acids were selected on the basis of pK_(a) and acceptability by regulatory authorities (Class 1, 2 and 3). See generally, Stahl, Heinrich P., Wermuth, Camile G., Editors, 2002. Handbook of Pharmaceutical Salts: Properties, Selection, and Use, Verlag Helvetica Chimica Acta. and Wiley-VCR. Weinheim. Germany and Switzerland; Bundavari, Susan, Editor, 1996, Merck Index, Twelfth Edition, Merck and Company, Inc., Whitehouse Station, New Jersey, USA.

As a general rule, salt formation is more likely to result when the difference between the pK_(a) of the acid and the pK_(a) of the anhydrous free base of Compound I (Form Ao) is greater than 2, whereas co-crystals are more likely when the pKa difference is less than 2. The application of co-crystal technologies has only recently become more recognized as a way to enhance the solubility and stability of certain APIs. The 24 acids listed in Table 2 were generally thought to be more likely to yield salt formation over cocrystal formation. Each Form A_(o)/acid combination was subject to maturation, slow cooling and evaporation crystallization techniques in 3 different solvents. In the experiments described herein reagent-grade acetone, chloroform, and tetrahydrofuran were used without further purification.

TABLE 2 Name, Pk_(a) Value And Melting Points Of Various Acids Acidity Melting point Acid (pKa) (° C.) Acetic acid 4.76 Liquid Ascorbic acid 4.17, 11.6 190-192 Benzoic acid 4.21   122.4 Citric acid 3.15, 4.77, 6.40 153 Ethanesulfonic acid 2.05 Liquid Fumaric acid 3.03, 4.44 287 Glutamic acid, DL 2.19, 4.25, 9.67 300 Glutaric acid 4.34, 5.42 95-98 Hippuric acid 3.55 187-188 Hydrobromic acid (48% aq) −6    Liquid Lactic acid 3.85   16.8 L - Tartaric acid 2.98, 4.34 171-174 L - Pyroglutamic acid 3.32 160-163 Maleic acid 1.92, 6.27 131-139 Malonic acid 2.83 135-136 Nicotinic acid 4.75 236 Octanoic acid 4.89 Liquid Orotic acid 5.85, 8.95 345 Ortho Phosphoric acid  2.12, 7.21, 12.67 Liquid Propionic acid 4.88 Liquid Sodium bisulfate monohydrate 1.9   74 Succinic acid 4.21, 5.64 185 Sulfuric acid −3    Liquid Toluenesulfonic acid, p- −2.8  106

X-Ray Powder Diffraction (XRPD)

Powder X-ray diffraction patterns were recorded on a PANalytical X Pert Pro diffractometer equipped with an X celerator detector using Cu Kα radiation at 45 kV and 40 mA. Kα1 radiation is obtained with a highly oriented crystal (Ge111) incident beam monochromator. A 10 mm beam mask, and fixed)(¼° divergence and anti-scatter)(½° slits were inserted on the incident beam side. A fixed 5 mm receiving slit and 0.04 Soller block were inserted on the diffracted beam side. The sample was rotated on a PANalytical PW3065/12 Spinner (15 revolutions I min). The typical X-ray powder pattern scan was collected from ca. 2 to 40° 28 with a 0.0080° step size and 96.06 sec counting time which resulted in a scan rate of approximately 0.5°/min. The samples were spread on silicon zero background (ZBG) plate for the measurement. For screening studies, the samples were spread on either ZBG or glass plates and were measured from ca. 2 to 35° 28 with a 0.0334° step size and 31.75 sec counting time which resulted in a scan rate of approximately 7.1°/min. Measurement of the Si reference standard before the data collection resulted in values for 28 and intensity that were well within the tolerances of 28.42<28<28.48 and significantly greater than the minimum peak height of 150 cps.

Variable Temperature X-Ray Powder Diffraction (VT-XRPD)

Variable temperature studies were performed with an Anton Paar TTK450 temperature chamber under computer control through an Anton Paar TCU100 temperature control unit. Typically the measurements were done with a nitrogen flow through the camera. Two measurement schemes were used, restricted and continuous. In the restricted mode, measurements were made after the TK450 chamber reached the requested temperature. In the continuous mode, the sample was heated at 10° C./minute and fast scans were measured as the temperature changed. After the requested temperature was reached, the sample was cooled at 35° C./minute and a slow scan measured 25° C. The temperatures chosen were based on DSC results. For the diffractometer set-up a 10 mm beam mask, 0.04 radian Soller block, fixed) (¼° divergence and anti-scatter)(½° slits were inserted on the incident beam side. A fixed 5 mm receiving slit, 0.04 radian Soller slits and a 0.02 mm Nickel filter were inserted on the diffracted beam side. The slow scans were collected from ca. 3 to 40° 28 with a 0.0080° step size and 100.97 sec counting time which resulted in a scan rate of approximately 0.5°/min. The fast scans were collected from ca. 3 to 30° 28 with a 0.0167° step size and 1.905 sec counting time which resulted in a scan rate of approximately 44°/min.

Differential Scanning Calorimetry (DSC)

Thermal curves were acquired using a Perkin-Elmer Sapphire DSC unit equipped with an autosampler running Pyris software version 6.0 calibrated with Indium prior to analysis. Solid samples of 1-10 mg were weighed into 20 μL aluminum samples pin with a pin-hole pan. The DSC cell was then purged with nitrogen and the temperature heated from 0 to 300° C. at 10° C. I min. Indium (Tm=156.6° C.; ΔHFUS=28.45 J g-1) was used for calibration.

Thermogravimetric Mass Spectrometry (TGA-MS)

Thermal curves were acquired using a Perkin-Elmer Pyris 1 TGA unit running Pyris software version 6.0 calibrated with alumel (95% nickel, 2% manganese, 2% aluminum and 1% silicon), nickel and calcium oxalate monohydrate. TGA samples between 1-5 mg were monitored for percent weight loss as heated from 25 to 250° C. at 10° C./min in a furnace purged with Helium at ca. 50 mL/min. To simultaneously follow the evolution of the gaseous decomposition products over the temperature range investigated, the thermobalance was connected to a Thermo Star Quadrupole Mass Spectrometer (Asslar, Germany). The transfer line to introduce gaseous decomposition products into the mass spectrometer was a deactivated fused silica capillary (SGE Analytical science, Fused Silica (100% Methyl Deactivated), 220 mm OD, 150 mm ID, Australia) temperature controlled to 200° C. to avoid possible condensation of the evolved gases. In this way the TGA weight loss and the mass spectrometric ion intensity curves of the selected ionic species could be recorded simultaneously.

Gravimetric Vapor Sorption (GVS)

GVS experiments have been carried out using the DVS-HT instrument (Surface Measurement Systems, London, UK). This instrument measures the uptake and loss of vapor gravimetrically using a recording ultra-microbalance with a mass resolution of ±0.1 μg. The vapor partial pressure (±1.0%) around the sample is controlled by mixing saturated and dry carrier gas streams using electronic mass flow controllers. The desired temperature is maintained at ±0.1° C. The samples (1-10 mg) were placed into the DVSHT and DVS-1 instruments at the desired temperature.

The sample was loaded and unloaded at 40% RH and 25° C. (typical room conditions). A moisture sorption isotherm was performed as outlined below (2 scans giving 1 complete cycle). The software uses a least squares minimization procedure together with a model of the mass relaxation, to predict an asymptotic value. The measured mass equilibration value must be within 2% of that predicted by the software before the next % RH value is selected. The minimum equilibration time was set to 1 hour and the maximum to 4 hours.

Fourier Transform Infrared (FTIR) Spectroscopy

Spectra were obtained using a Thermo Electron-Nicolet Avatar 370 DTGS instrument with the Smart Orbit ATR attachment containing a diamond crystal window. Thermo Electron Omnic™ software (version 3.1) was used to compute the spectrum from 4000 to 400 cm-1 from the initial interferogram. A background scan was collected before spectral resolution and averaged. Assignments of the absorption frequencies were made using Know It All software (version 8.0).

Optical Microscopy (OM)

Microscopic observation of the sample morphology was performed using an Olympus B60 polarized light microscope. Samples were suspended in mineral oil and compressed on a glass slide with a cover slip prior to observation. Images were taken with a FW-24 (PAX CAM) camera. A 10× objective coupled with an additional 10× magnification from the microscope optics gave a total magnification of 100×. The Pax-it software (version 6.2) was used to analyze and photograph the images.

Identity, Assay, and Purity by HPLC

Typically 1-5 mg of samples were diluted to 10 mL with sample solvent (1:1 (v:v) Mobile phase A:Mobile phase B) and the assay concentrations were determined from an average of duplicate injections using the following HPLC method. The purity and impurity analyses are done using conventional HPLC.

Column: Zorbax SB-CN, 1.8 μm, 50 × 4.6 mm (length × ID) Col. Pre-Filter: OptiSolv EXP 0.2 μm Column Temp: 50° C. Detector: UV, 280 nm Inject: 10 μL Flow rate: 0.8 mL/min. Mobile phases: A. 15 mM Ammonium Acetate (aq.), pH = 4.0 B 100% Methanol Gradient: Time (min.) % A % B 0.0 80 20 4.0 50 50 9.5 50 50 14.0 20 80 18.0 20 80 18.5 80 20 22.0 80 20

Determination of Solid-State Stability

Samples of Compound I free base and its salts (approximately 10 mg each) were stored at 40° C./75% RH in open glass vials (4 cm³) over four weeks without desiccant.

Solubility of Form A₀

The following procedure was used to assess the solubility of the anhydrous free base of Compound I (Form A₀) in a range of nine organic solvents listed in Table 3. Using 1.8 mL HPLC vials, approximately 10 mg of Form A₀ was stirred at the boiling point in 200 μL of nine different solvents. If the solid did not dissolve, an additional 100, 200 or 500 μL of solvent was added with heating to the boiling point. The additions were stopped when the solid dissolved or when 1000 μL had been dispensed. The best solubility for Form Ao was observed in acetone, chloroform, and tetrahydrofuran. Methyl t-butyl ether was chosen as an anti-solvent (<10 mg/mL).

TABLE 3 Solubility Of Form A₀ In Different Solvents Boiling Point Solubility Estimate at Solvent (° C.) The Boiling Point Acetone 56.5 >50 mg/mL Acetonitrile 82.0 <20 mg/mL Chloroform 61.2 >50 mg/mL Ethyl Acetate 77.1 <30 mg/mL Methanol 64.7 <20 mg/mL Methyl-t-butyl Ether 55.2 <10 mg/mL Dichloromethane 40.0 >20 mg/mL Tetrahydrofuran 66.0 >50 mg/mL Toluene 110.6 <30 mg/mL

Characterization of Salts of Compound I

Crystallizations studies were performed on Form Ao to investigate salt formation. Maturation, slow cooling and evaporation techniques were employed to obtain different salts of Compound I. When possible, full characterization was performed on the new forms that were generated. This characterization consisted of: X-ray powder diffraction and variable-temperature X-ray powder analysis; thermal analysis; gravimetric vapor sorption; Fourier transform infrared spectroscopy, and optical microscopy.

Maturation Experiments with Acetone

For each of the acids listed below, the quantity calculated to give approximately 1.05 equivalents of acid per 20 mg of free base was weighed into a glass vial. If the acid was liquid, the density was used to determine a volume necessary to give equal mass. One mL of Form Ao dissolved in acetone (20 mg/1 mL) was added to the vial. The resulting mixtures were slurried for a total of 96 hours with alternating 4 hour periods at 50° C. and 5° C. (±0.5° C./min) using a HEL Polyblock™ Unit. The solid material was isolated by filtration, dried at 40° C. for 18 hours under house vacuum and analyzed by XRPD, DSC, and TGA. A summary of the results are shown in Table 4. The crystallization experiments were carried out in glass vials (1.5 mL, 32×11.6 mm).

TABLE 4 Maturation Study Results For Acetone Salt X-ray Result DSC TGA* Hydrobromic New pattern 229.2° C., 238.9° C. 0.04% acid (48% aq) Malonic acid New pattern 171.7° C. 1.7% Ortho-Phosphoric New pattern 186.3° C. 0.1% acid (85%) *Weight loss from 25 to 150° C. Maturation Experiments with Chloroform

For each of the acids listed below, the quantity calculated to give approximately 1.05 equivalents of acid per 20 mg of free base, was weighed into a glass vial. If the acid was liquid, the density was used to determine a volume necessary to give equal mass. One mL of Form Ao dissolved in chloroform (20 mg I 1 mL) was added to the vial. The resulting mixtures were slurried for a total of 96 hours with alternating 4 hour periods at 50° C. and 5° C. (±0.5° C./min) using a HEL Polyblock™ Unit. The solid material was isolated by filtration, dried at 40° C. for 18 hours under house vacuum and analyzed by XRPD, DSC, and TGA. The results are shown in Table 5. The crystallization experiments were carried out in glass vials (1.5 mL, 32×11.6 mm).

TABLE 5 Maturation Study Results For Chloroform Salt X-ray Result DSC TGA* Hydrobromic New pattern 68.7° C., 187.4° C., 3.7% acid (48% aq) 210.3° C. Malonic acid New pattern 52.52° C., 131.8° C., 14.0% 163.0° C. Ortho-Phosphoric Amorphous 142.1° C. 10.8% acid (85%) *Weight loss from 25 to 150° C. Maturation Experiments with Tetrahydrofuran

For each of the acids listed below, the quantity calculated to give approximately 1.05 equivalents of acid per 20 mg of free base, was weighed into a glass vial. If the acid was liquid, the density was used to determine a volume necessary to give equal mass. One mL of Form Ao dissolved in tetrahydrofuran (20 mg/1 mL) was added to the vial. The resulting mixtures were slurried for a total of 96 hours with alternating 4 hour periods at 50° C. and 5° C. (±0.5° C./min) using a HEL Polyblock™ Unit. The solid material was isolated by filtration, dried at 40° C. for 18 hours under house vacuum and analyzed by XRPD, DSC, and TGA. The results are shown m Table 6. The crystallization experiments were carried out m glass (1.5 mL, 32×11.6 mm).

TABLE 6 Maturation Study Results For Tetrahydrofuran Salt X-ray Result DSC TGA* Hydrobromic acid (48% aq) New pattern 189.2° C. weak, 0.2% 227.8° C. Malonic acid New pattern 169.7° C. 3.4% Ortho-Phosphoric acid (85%) New pattern 180.5° C. 0.4% *Weight loss from 25 to 150° C. Slow Cool Experiments with Acetone

For each of the acids listed in the table below, the quantity calculated to give approximately 1.05 equivalents of acid per 20 mg of free base, was weighed into a glass vial. If the acid was liquid, the density was used to determine a volume necessary to give equal mass. One mL of Form Ao dissolved in acetone (20 mg I 1 mL) was added to the vial. The samples were heated from 20° C. to 80° C. at a rate of 5° C./min and after 60 minutes cooled at a slow rate (−0.25° C./min) to a final temperature of 5° C. and kept at that temperature for 18 h using the HEL Polyblock™ Unit. The solid material was isolated by filtration, dried at 40° C. for 18 hours under house vacuum and analyzed by XRPD, DSC, and TGA. The results are shown in Table 7. The crystallization experiments were carried out in glass vials (1.5 mL, 32×11.6 mm).

TABLE 7 Maturation Study Results For Acetone Salt X-ray Result DSC TGA* Hydrobromic acid (48% aq) New pattern 228.3° C. 0.2% Malonic acid New pattern 61.5° C., 167.7° C. 2.7% Ortho-Phosphoric acid New pattern 58.0° C., 185.3° C. 0.9% (85%) *Weight loss from 25 to 150° C. Slow Cool Experiments with Chloroform

For each of the acids listed in the table below, the quantity calculated to give approximately 1.05 equivalents of acid per 20 mg of free base was weighed into a glass vial. If the acid was liquid, the density was used to determine a volume necessary to give equal mass. One mL of Form Ao dissolved in chloroform (20 mg I 1 mL) was added to the vial. The samples were heated from 20° C. to 80° C. at a rate of 5° C./min and after 60 minutes cooled at a slow rate (−0.25° C./min) to a final temperature of 5° C. and kept at that temperature for 18 h using the HEL Polyblock™ Unit. The solid material was isolated by filtration, dried at 40° C. for 18 hours under house vacuum and analyzed by XRPD, DSC, and TGA. The results are shown in Table 8. The crystallization experiments were carried out in glass vials (1.5 mL, 32×11.6 mm).

TABLE 8 Maturation Study Results For Chloroform Salt X-ray Result DSC TGA* Hydrobromic acid New pattern 181.9° C., 221.9° C. 1.1% (48% aq) Malonic acid New pattern 49.2° C., 127.3° C., 12.5% 160.8° C. Ortho-Phosphoric acid Amorphous 180.5° C. 7.9% (85%) *Weight loss from 25 to 150° C. Slow Cool Experiments with Tetrahydrofuran

For each of the acids listed in the table below, the quantity calculated to give approximately 1.05 equivalents of acid per 20 mg of free base, was weighed into a glass vial. If the acid was liquid, the density was used to determine a volume necessary to give equal mass. One mL of Form Ao dissolved in tetrahydrofuran (20 mg/1 mL) was added to the vial. The samples were heated from 20° C. to 80° C. at a rate of 5° C./min and after 60 minutes cooled at a slow rate (−0.25° C./min) to a final temperature of 5° C. and kept at that temperature for 18 h using the HEL Polyblock™ Unit. The solid material was isolated by filtration, dried at 40° C. for 18 hours under house vacuum and analyzed by XRPD, DSC, and TGA. The results are shown in Table 9. The crystallization experiments were carried out in glass vials (1.5 mL, 32×11.6 mm).

TABLE 9 Slow Cool Study Results for Tetrahydrofuran Salt X-ray Result DSC TGA* Hydrobromic acid (48% aq) New pattern 227.9° C. 0.6% Malonic acid New pattern 167.1° C., 3.1% 198.4° C. Ortho-Phosphoric acid (85%) New pattern 188.8° C. 0.7% *Weight loss from 25 to 150° C.

Evaporation Experiments in Acetone

For each of the acids listed in the table below, the quantity calculated to give approximately 1.05 equivalents of acid per 20 mg of free base was weighed into a glass vial. If the acid was liquid, the density was used to determine a volume necessary to give equal mass. One mL of Form A₀ dissolved in acetone (20 mg/1 mL) was added to the vial. Approximately 20 mg of Form A₀ was added to the vial (20 mL, 26×58 mm). The solutions or mixtures were allowed to slowly evaporate to dryness under ambient conditions. Resulting solids were analyzed by XRPD, DSC, and TGA. The results are shown in Table 10.

TABLE 10 Evaporation Study Results for Acetone Salt X-ray Result DSC TGA* Hydrobromic acid (48% aq) New pattern 226.4° C. 0.1% Malonic acid New pattern 70.1° C., (—) 114.7° C., 171.9° C. Ortho-Phosphoric acid (85%) No peaks 75.9° C., 3.7% 141.1° C. *Weight loss from 25 to 150° C.

Evaporation Experiments in Chloroform

For each of the acids listed in the table below, the quantity calculated to give approximately 1.05 equivalents of acid per 20 mg of free base was weighed into a glass vial. If the acid was liquid, the density was used to determine a volume necessary to give equal mass. Approximately 20 mg of Form A₀ was added to the vial (20 mL, 26×58 mm). Chloroform was added in 0.5 to 1.0 mL increments followed by heating with stirring to the boiling point. If a clear solution was achieved, the incremental additions were stopped. If a clear solution was not observed when a total of 10 mL of solvent was added, the mixture was syringe filtered (5μ Nylon membrane) into a clean vial. The solutions were allowed to slowly evaporate to dryness under ambient conditions. Resulting solids were analyzed by XRPD, DSC, and TGA. The results are shown in Table 11.

TABLE 11 Evaporation Study Results Salt X-ray Result DSC TGA* Hydrobromic acid Amorphous 180.0° C. 2.4% 2.4% Malonic acid New pattern 128.7° C., 27.9% 137.9° C., 161.8° C. Ortho-Phosphoric acid New pattern 178.8° C. 9.2% *Weight loss from 25 to 150° C.

Evaporation Experiments in Tetrahydrofuran

For each of the acids listed in the table below, the quantity calculated to give approximately 1.05 equivalents of acid per 20 mg of free base was weighed into a glass vial. If the acid was liquid, the density was used to determine a volume necessary to give equal mass. Approximately 20 mg of Form Ao was added to the vial (20 mL, 26×58 mm). Tetrahydrofuran was added in 0.5 to 1.0 mL increments followed by heating with stirring to the boiling point. If a clear solution was achieved, the incremental additions were stopped. If a clear solution was not observed when a total of 10 mL of solvent was added, the mixture was syringe filtered (5μ Nylon membrane) into a clean vial. The solutions were allowed to slowly evaporate to dryness under ambient conditions. Resulting solids were analyzed by XRPD, DSC, and TGA. The results are shown in Table 12.

TABLE 12 Evaporation Study Results for Tetrahydrofuran Salt X-ray Result DSC TGA* Hydrobromic acid New pattern 225.1° C. 1.7% Malonic acid New pattern 65.6° C., 168.3° C. 4.3% Ortho-Phosphoric acid Amorphous  62.8° C. 6.2% *Weight loss from 25 to 150° C.

Summary of Salt Results

One stable crystalline form of Form A₀ was identified (See Table 13). In several cases, Form Ao precipitated from solution with no indication of salt formation. Data pertaining to four salts is shown in Tables 12 and 14. A detailed characterization of these salts is also described in this application.

TABLE 13 Characterization Data Form A₀ Form XRPD DSC (° C.) TGA¹ XGVS² XRPD³ Purity (%) A₀ Crystalline 236.0 0.2 1.3 No 98.3 change N/A = Not Available ¹Weight loss 25° C. to 120° C. ²Percent increase in mass at 90% RH ³After GVS analysis

TABLE 14 Characterization Data For Isolated Salts DSC Purity Salt XRPD (° C.) TGA¹ GVS² XRPD³ (%) Bromide A₁ Crystalline 230.9 0.1 1.0 No change 98.4 Chloride A₁ Crystalline 236.1 0.2 1.7 No change N/A Malonate A₁ Crystalline 171.7 1.7 N/A N/A 98.6 Phosphate A₁ Crystalline 186.3 0.1 2.7 No change 95.8 N/A = Not Available ¹Weight loss 25° C. to 120° C. ²Percent increase in mass at 90% RH ³After GVS analysis

Solid State Analysis Compound I Free Base, Form A₀

Preparation from Form A₀

To a 10 L Chemglass jacketed reactor with N₂ inlet/outlet was added compound 2 (200.0 g, 637 mmol), compound 3 (177.0 g, 596 mmol) and 4-Dimethylaminopyridine (DMAP) (2.88 g) followed by 4.0 L of isopropyl acetate. The internal temperature was raised to 70° C. and heated for 9 hours. The reaction remained a slurry throughout the reaction and HPLC showed no compound 2 remaining after heating for that period. Next, 2.0 L of heptane were added at 70° C. and the reaction cooled to 20° C. The solids were stirred for 1 hour, filtered and the cake washed with 2.0 L of 1:1 isopropyl acetate/heptanes. The white solids were placed in an oven with N2 bleed at 55° C. under 75 mbar vacuum. The resulting solids weighed 295 g (96% yield) of Form A₀ with 99.3% purity by HPLC.

Characterization by XRPD

The X-ray diffraction pattern characteristic of the crystalline Form A_(o) is shown in 5 Table 15 and FIG. 1.

TABLE 15 Select Two Theta Positions (2θ), D-Spacings (d) And Relative Intensities (I) Of XRPD d-spacing Rel. Int. No. Pos. [2θ.] [Å] [%] 1 4.77 18.52 100 2 9.76 9.06 10 3 9.80 9.02 9 4 10.02 8.82 11 5 11.37 7.78 11 6 12.56 7.04 8 7 14.30 6.19 27 8 14.39 6.15 36 9 14.70 6.02 19 10 15.82 5.60 13 11 19.10 4.64 5 12 19.48 4.55 13 The highest peak (intensity 100%) is set in bold letters.

Characterization by VT-XRPD

Slow scans were measured after heating to the requested temperature and cooling back to 25° C. The initial scan matches the pattern for the Form A₀. After heating to 200° C., there are changes in intensity, but not in peak positions (FIG. 2). After heating to 255° C., the XRFD pattern is featureless and the sample on the VT plate was a golden hued solid in the shape of a droplet. All measurements were made with a flow of nitrogen gas through the sample stage.

Characterization of Form A₀ by Thermal Analysis

Form A₀ shows a single peak at ca. 214.0° C. with an ΔHFus of 93.0 J/g. No loss of mass was detected by TGA. The existence of a desolvation process was discounted because a minimal loss of weight was detected by TGA (FIG. 3).

Characterization by Water Sorption of Form A₀ (Dm/Dt Mode)

Form A₀ from 40 to about 90% RH has a moisture uptake of less than 1.3% (w/w). In the second sorption step, the sample experienced a slow uptake of water (FIG. 4). XRPD analysis was performed on the sample after two cycles of the GVS experiment. The XRFD pattern of this material compares nicely to the pattern of the material before GVS (FIG. 5).

Characterization by FTIR Spectroscopy

The Fourier transform infrared spectrum of Form Ao and its characteristic bands are provided in Table 16 and FIG. 6.

TABLE 16 Fourier Transform Infrared Bands Of Form A₀ Infrared Frequency, cm⁻¹ Assignment 3359.1 NH stretch PH—NH—R 3096.5.0 Aromatic CH stretch 2940.8 R—CH3 asym stretch 2838.5 R2—NH2+ stretch 1733.3 C═0 stretch urea 1607.3 NH2 def Amide II 1562.3 Aromatic 1414.8 C—N stretch Amide 1249.5 Ph—O—C ether, asym stretch 1132.5 CH2—O—CH2 ether, asym stretch 1088.4 Ph—O—C ether, sym stretch 826.2 Ph—O—C ether, sym stretch 679.7 C—H rocking

Optical Microscopy

The sample of Form Ao showed small needles (magnification 100×) and the material exhibited birefringence (FIG. 7).

Bromide Form A₁ Preparation Crystallization by Maturation

Approximately 1.05 equivalents of the calculated quantity of hydrobromic acid (48%) to react with 80 mg of free base are weighed into a glass vial in 40000 μL of THF. The sample was heated from 20° C. to 80° C. at a rate of 5° C./min and after 60 minutes cooled at a slow rate (0.25° C./min) to a final temperature of 5° C. and kept at that temperature for 18 hours using the HEL Polyblock™ Unit. The crystallization experiment was carried out in a glass vial (4.0 mL; 46×14.5 mm). The solid material was isolated by filtration and dried at 40° C. for 18 hours under house vacuum. The sample was analyzed by XRPD, DSC, TGA, FTIR, and OM.

Characterization by XRPD

The peaks and X-ray diffraction pattern characteristic of the crystalline bromide Form A1 are shown in Table 17 and FIG. 8.

TABLE 17 Select Two Theta Positions (28). D-Spacings (D) And Relative Intensities (I) Of XRPD No. Pos. [°2Th.] d-spacing [Å] Rel. Int. [%] 1 2.02 43.68 10 2 5.64 15.67 100 3 8.15 10.85 23 4 9.87 8.95 24 5 11.16 7.92 15 6 13.85 6.39 51 7 16.29 5.44 9 8 17.15 5.17 6 9 18.62 4.76 49 10 19.68 4.51 5 11 22.30 3.98 31 12 23.75 3.74 14 13 27.66 3.22 5 14 29.18 3.06 7 15 34.75 2.58 5

Characterization of Bromide Form A₁ by Thermal Analysis

Bromide Form A₁ shows a single peak at ca. 230.9° C. with an enthalpy of fusion (ΔHFus) of 123.6 Jig. Bromide Form A₁ when studied by TGA demonstrated an average weight loss of 0.07% between 25° C. and 150° C. (FIG. 9).

Characterization by Water Sorption of Bromide Form A₁ at 25° C. (Dm/Dt Mode)

The amount of moisture adsorbed at 75% RH was less than 0.7% and approximately 1% at 90% RH. The adsorption and desorption curves overlap suggesting that Form A1 is not hygroscopic (FIG. 10 and FIG. 11). XRPD analysis was performed on the sample after the two cycle Gravimetric Vapor Sorption experiment. The XRPD pattern of this material compares nicely to the pattern of the material before GVS (FIG. 12).

Characterization by FTIR Spectroscopy

The Fourier transform infrared spectrum of bromide Form A₁ and its characteristic bands are provided in Table 18 and FIG. 13.

TABLE 18 FTIR Bands Of Bromide Form A₁ Infrared Frequency, cm−1 Assignment 3243.5 NH stretch Ph—NH—R 3056.6 Aromatic CH stretch 2949.8 R—CH₃ asym stretch 2749.6 CH stretch 1713.7 C═0 stretch Urea 1632.4 NH₂ def Amide II 1602.6 R₂—NH₂ ⁺ def 1417.7 C—N stretch Amide 1216.8 Ph—O—C ether, asym stretch 1132.8 CH₂—O—CH₂ ether, asym stretch 1065.4 Ph—O—C ether, sym stretch 873.4 Ph—O—C ether, sym stretch 647.1 CH rock

Optical Microscopy

The sample of bromide Form A₁ showed aggregates and small needles (magnified 100×). The material exhibited birefringence (FIG. 14).

Chloride Form A₁ Preparation Crystallization

The chloride Form A₁ was formed by dissolving the Form A₀ in tetrahydrofuran/isopropyl acetate. After the addition of 1.3 equivalents of 5-6N hydrogen chloride in isopropanol, the mixture was stirred overnight. The isolated yield was 96.6%. The sample was analyzed by XRPD, DSC, TGA, FTIR, and OM.

Characterization by XRPD

The peaks and X-ray diffraction pattern characteristic of the crystalline chloride Form A₁ are shown in Table 19 and FIG. 15.

TABLE 19 Select Two Theta Positions (2θ). D-Spacings (d) And Relative Intensities (I) Of XRPD Pos. d-spacing Rel. Int. No. [°2Th.] [Å] [%] 1 5.67 15.59 100 2 8.55 10.34 29 3 9.96 8.87 26 4 10.46 8.45 19 5 11.24 7.87 8 6 12.30 7.19 12 7 14.10 6.28 16 8 14.48 6.11 83 9 14.81 5.98 22 10 15.35 5.77 22 11 15.89 5.57 44 12 17.08 5.19 15 13 17.37 5.10 10 14 17.73 5.00 15 15 19.36 4.58 27 16 20.96 4.24 13 17 21.48 4.13 11 18 21.66 4.10 8 19 22.50 3.95 67 20 22.87 3.89 8 21 22.98 3.87 6 22 24.08 3.69 8 23 24.57 3.62 8 24 26.03 3.42 5 25 26.23 3.39 5 26 26.83 3.32 23 27 27.56 3.23 25 28 29.07 3.07 8 29 29.99 2.98 15 30 20.96 4.24 13 The highest peak (intensity 100%) is set in bold letters.

Characterization by VT-XRPD

No solid-solid transformation takes place m the between 25° C. and 200° C. for Chloride Form A₁. Upon heating to 245° C., the sample melts with no indication of recrystallization on cooling to 25° C. (FIG. 16).

Characterization of Chloride Form A₁ by Thermal Analysis

The chloride Form A₁ shows a single peak at ca. 236.1° C. with an ΔHFus of 256.1 J/g. TGA measurement demonstrated an average weight loss of 0.2% between 25° C. and 150° C. (FIG. 17).

Characterization by Water Sorption of Chloride Form A₁ at 25° C. (Dm/Dt Mode)

The first adsorption curve (FIG. 18) exhibits a weight increase of 1.7% through 90% RH. The second cycle for Form A₁ closely reproduces the first cycle. No form change occurred during the GVS cycles. The sample was the same crystalline form after the GVS experiment as shown by the XRPD patterns in FIG. 19.

Characterization of Chloride Form A₁ by FTIR

The FTIR spectrum for Form A₁ is shown in FIG. 20, and the proposed peak assignments are given in Table 20.

TABLE 20 FTIR Bands For Chloride Form A₁ Infrared Frequency, cm⁻¹ Assignment 3199.0 NH stretch; Urea 3061.1 CH stretch; m-distributed aromatic 3007.7 CH stretch; 1,2,4,5-substituted aromatic 2940.9 R—CH₃ asym stretch 2709.5 NH stretch; aromatic NH⁺ 1711.2 C═O stretch; Urea 1632.6 Aromatic ring stretch 1602.9 Aromatic ring stretch 1541.9 NH def Urea 1499.6 Aromatic ring stretch 1391.1 N—C—N stretch Urea 1283.4 Ph—O—C ether, asym stretch 1133.1 C—F stretch 1029.5 Ph—O—C ether, sym stretch 885.2 Ph—O—C ether, sym stretch 803.3 Aromatic ring def 700.5 Aromatic ring bend

Optical Microscopy

The sample of chloride Form A₁ showed aggregates and small needles (magnified 100×). The material exhibited birefringence (FIG. 21).

Malonate Form A₁ Preparation Crystallization by Maturation

Approximately 1.05 equivalents of the calculated quantity of malonic acid to react with 80 mg of Form A₀ were weighed into a glass vial with 40000 μL of THF. This mixture was slurried for a total of 48 hours with alternating 4 hour periods at 50° C. and 5° C. (±0.5° C./min) using the HEL Polyblock™ Unit. The crystallization experiments were carried out in glass vials (4.0 mL. 346×14.5 mm). The solid material was isolated by filtration and dried at 40° C. for 18 hours under house vacuum. The sample was analyzed by XRPD, DSC, TGA, GVS, FTIR, and OM.

Characterization by XRPD

The peaks and X-ray diffraction pattern characteristic of the crystalline malonate Form A1 are shown in Table 21 and FIG. 22.

TABLE 21 Select Two Theta Positions (2θ). D-Spacings (d) And Relative Intensities (I) Of XRPD Pos. d-spacing Rel. Int. No. [°2Th.] [Å] [%] 1 3.57 24.72 100 2 3.66 24.12 72 3 5.97 14.80 6 4 7.08 12.48 26 5 7.18 12.31 11 6 10.16 8.70 7 7 10.44 8.46 40 8 10.59 8.34 32 9 11.05 8.00 14 10 12.16 7.27 5 11 12.89 6.86 8 12 14.12 6.27 29 13 15.30 5.79 8 14 16.20 5.47 6 15 16.64 5.32 6 16 17.36 5.10 7 17 17.67 5.01 47 8 21.21 4.18 20 19 22.32 3.98 6 20 25.73 3.46 12 21 26.03 3.42 38 22 26.30 3.39 19 23 26.93 3.31 36 24 27.64 3.22 5 25 28.03 3.18 15 26 28.42 3.14 6 The highest peak (intensity 100%) is set in bold letters.

Characterization of Malonate Form A₁ by Thermal Analysis

Malonate Form A₁ gave a single peak at ca. 171.7° C. with an ΔHfus of 140.6 J/g. Malonate Form A₁ when studied by TGA demonstrated an average weight loss of 1.7% between 25° C. and 150° C. (FIG. 23).

Characterization by Water Sorption of Malonate Form A₁ at 25° C. (Dm/Dt Mode)

There is a steady uptake in water over the RH range of 0-90%. Surface adsorption with limited bulk absorption is occurring. The total uptake is <4%. No form change occurred during the GVS cycles.

Characterization by Water Sorption of Malonate Form A₁ at 25° C. (Dm/Dt Mode)

The FTIR spectrum for malonate Form A1 is shown in FIG. 24, and the proposed peak assignments are given in Table 22.

TABLE 22 FTIR Bands For Malonate Form A₁ Infrared Frequency, cm⁻¹ Assignment 3136.7 NH stretch; Urea 3061.1 CH stretch; m-distributed aromatic 3007.7 CH stretch; 1,2,4,5-substituted aromatic 2936.5 R—CH₃ asym stretch 2825.5 NH stretch; aromatic NH⁺ 1708.3 C═O stretch; Urea 1632.6 Aromatic ring stretch 1608.1 Aromatic ring stretch 1575.4 NH def Urea 1515.1 Aromatic ring stretch 1398.4 N—C—N stretch Urea 1283.2 Ph—O—C ether, asym stretch 1131.8 C—F stretch 1088.7 Ph—O—C ether, sym stretch 993.7 Ph—O—C ether, sym stretch 821.9 Aromatic ring def 733.6 Aromatic ring bend

Optical Microscopy

The sample of malonate Form A₁ showed aggregates (magnified 100×) and the material exhibited birefringence (FIG. 25).

Phosphate Form A₁ Preparation Crystallization by Maturation

Approximately 1.05 equivalents of the calculated quantity of ortho-phosphoric acid to react with 80 mg of Form A₀ were added to a glass vial with 2 mL of acetone. This mixture was slurried for a total of 48 hours with alternating 4 hour periods at 50° C. and 5° C. (±0.5° C./min) using the HEL Polyblock™ Unit. The crystallization experiments were carried out in glass vials (4 0 mL. 46×14.5 mm). The solid material was isolated by filtration and dried at 40° C. for 18 hours under house vacuum. The sample was analyzed by XRPD, DSC, TGA, GVS, FTIR, and OM.

Characterization by XRPD

The peaks and X-ray diffraction pattern characteristic of the crystalline phosphate Form A1 are shown in Table 23 and FIG. 26.

TABLE 23 Select Two Theta Positions (2θ). D-Spacings (i) And Relative Intensities (I) Of XRPD No. Pos. [2θ.] d-spacing [Å] Rel. Int. [%] 1 3.26 27.11 22 2 6.47 13.66 100 3 9.63 9.18 19 4 11.55 7.66 5 5 12.89 6.86 24 6 15.54 5.70 38 7 16.09 5.50 15 8 18.49 4.79 6 9 21.55 4.12 7 The highest peak (intensity 100%) is set in bold letters.

Characterization of Phosphate Form A₁ by Thermal Analysis

Phosphate Form A₁ shows a single peak at ca. 186.3° C. with an enthalpy of fusion (ΔHFus) of 78.7 J/g (FIG. 27). Phosphate Form A₁ when studied by TGA demonstrated an average weight loss of 0.12% between 25° C. and 150° C.

Characterization by Water Sorption of Phosphate Form A₁ at 25° C. (Dm/Dt Mode)

The amount of moisture adsorbed at 75% RH was less than 1.8% and approximately 2.7% at 90% RH. The adsorption and desorption curves overlap suggesting that Compound I phosphate Form A1 is not hygroscopic (FIG. 28 and FIG. 29). XRPD analysis was performed on the sample after the two cycles of the GVS experiment. The XRPD pattern of this material compares nicely to the pattern of the material before GVS (FIG. 30).

Characterization of Phosphate Form A₁ by FTIR

The FTIR spectrum for phosphate Form A1 is shown m FIG. 31, and the proposed peak assignments are given in Table 24.

TABLE 24 FTIR Bands For Phosphate Form A₁ Infrared Frequency, cm⁻¹ Assignment 3288.0 NH stretch; Urea 3216.8 CH stretch; m-distributed aromatic 3087.8 CH stretch; 1,2,4,5-substituted aromatic 2927.6 R—CH₃ asym stretch 2838.6 NH stretch; aromatic NH⁺ 1726.1 C═O stretch; Urea 1641.5 Aromatic ring stretch 1613.0 Aromatic ring stretch 1510.0 NH def Urea 1494.2 Aromatic ring stretch 1421.2 N—C—N stretch Urea 1285.4 Ph—O—C ether, asym stretch 1133.5 C—F stretch 1002.3 Ph—O—C ether, sym stretch 984.0 Ph—O—C ether, sym stretch 861.6 Aromatic ring def

Optical Microscopy

The sample of Phosphate Form A₁ showed aggregate and small particles (magnified 100×). The material exhibited birefringence (FIG. 32).

Kinetic Solubility Measurement

Solubility measurements of Compound I free base, Form A₀, and four salts were performed in pure water.

Sample Solution Preparation

The free base and the salts listed in the table below were added in excess (saturation) to water in a 2.0 mL glass vial. The samples were put on an end-to-end rotator (50 rpm) at ambient room temperature up to 20 minutes. After 20 minutes, a sampling was taken for HPLC analysis.

The results are presented in Table 25. The aqueous solubility measurement confirmed the chloride salt was the best salt for dissolution in pure water (pH=7).

TABLE 25 Aqueous Solubility Measurement Of The Free Base And The Salts Material tested mg/mL pH Free base A₀ <0.01 7.4 Bromide A₁ 0.1 6.6 Chloride A₁ 0.56 7.3 Malonate A₁ 0.07 6.6 Phosphate A₁ 0.09 6.8 The amount of compound dissolved in water is expressed as free base.

Relationship Between Solid State Forms Solid State Stress Stability

Stress stability studies were performed to get a timely impression of the influence of temperature and humidity on Form stability.

Form A₀ and Chloride Form A₁

In the solid state at standard ICH stressed conditions of 40° C./75% relative humidity without desiccant, free base Form Ao and chloride Form A1 were stable for 28 days (Table 26 and Table 27).

TABLE 26 Stability Data For Form A₀ At 40° C./75% RH Sample DSC TGA HPLC Assay Area ID Time/days XRPD (°) (%*) (%) Purity (%) 248-0 0 Form A₀ 214.0 1.8 100.0 98.3 248-6 6 Form A₀ 215.4 0.2 102.3 98.5 248-14 14 Form A₀ 215.5 0.2 100.5 98.5 248-28 28 Form A₀ 215.7 0.01 102.4 98.2 *weight loss 25° C. to 150° C.

TABLE 27 Stability Data For Chloride Form A₁ At 40° C./75% RH Sample DSC TGA HPLC Assay Area ID Time/days XRPD (°) (%*) (%) Purity (%) 274-0 0 Form A₁ 228.9 0.8 99.9 99.5 274-7 7 Form A₁ 224.7 0.1 98.3 98.7 274-14 14 Form A₁ 229.2 0.1 98.7 97.6 274-8 28 Form A₁ 228.5 0.3 100.4 96.4 *weight loss 25° C. to 150° C. 

1.-18. (canceled)
 19. A salt of N-[3-[(6,7-dimethoxy-4-quinazolinyl)oxy]phenyl]-N′-[5-(2,2,2-trifluoro-1,1-dimethylethyl)-3-isoxazolyl]-urea, wherein said salt has a solubility expressed as an amount of free base in water at pH 7 and at ambient room temperature of greater than 0.01 mg per mL.
 20. A salt according to claim 19, wherein said salt has a solubility expressed as an amount of free base in water at pH 7 equal to or greater than 0.07 mg per mL.
 21. A salt according to claim 19, wherein said salt has a solubility expressed as an amount of free base in water at pH 7 equal to or greater than 0.09 mg per mL.
 22. A salt according to claim 19, wherein said salt has a solubility expressed as an amount of free base in water at pH 7 equal to or greater than 0.10 mg per mL.
 23. A salt of N-[3-[(6,7-dimethoxy-4-quinazolinyl)oxy]phenyl]-N′-[5-(2,2,2-trifluoro-1,1-dimethylethyl)-3-isoxazolyl]-urea, wherein said salt is selected from the hydrobromide salt, the hydrochloride salt, the malonate salt and the phosphate salt.
 24. A salt according to claim 23, wherein said salt is the hydrochloride salt.
 25. A crystalline form of the hydrochloride salt of N-[3-[(6,7-dimethoxy-4-quinazolinyl)oxy]phenyl]-N′-[5-(2,2,2-trifluoro-1,1-dimethylethyl)-3-isoxazolyl]-urea, wherein said crystalline form is characterized by an x-ray powder diffraction pattern comprising a peak at a 2-theta value of about 5.67±0.2 degrees.
 26. A crystalline form according to claim 25, wherein said x-ray powder diffraction pattern further comprises a peak at a 2-theta value of about 14.48±0.2 degrees.
 27. A crystalline form according to claim 26, wherein said x-ray powder diffraction pattern further comprises a peak at a 2-theta value of about 15.89±0.2 degrees.
 28. A crystalline form according to claim 27, wherein said x-ray powder diffraction pattern further comprises peaks at 2-theta values of about 8.55±0.2 degrees, 9.96±0.2 degrees, 19.36±0.2 degrees, 26.83±0.2 degrees, and 27.56±0.2 degrees.
 29. A crystalline form according to claim 25, wherein said crystalline form is further characterized by exhibiting a peak in a differential scanning calorimetry scan of about 236° C.
 30. A pharmaceutical composition, comprising the hydrochloride salt of N-[3-[(6,7-dimethoxy-4-quinazolinyl)oxy]phenyl]-N′-[5-(2,2,2-trifluoro-1,1-dimethylethyl)-3-isoxazolyl]-urea and a pharmaceutically acceptable excipient.
 31. A pharmaceutical composition according to claim 30, wherein said composition is in a form suitable for oral administration to a subject.
 32. A pharmaceutical composition according to claim 31, wherein said composition is in the form of a tablet, pill, powder, capsule, or troche.
 33. A pharmaceutical composition according to claim 32, wherein said composition is in the form of a tablet, pill, or capsule.
 34. A pharmaceutical composition according to claim 33, wherein said composition is in the form of a tablet or capsule.
 35. A pharmaceutical composition according to claim 34, wherein said composition is in the form of a tablet.
 36. A pharmaceutical composition according to claim 34 wherein said composition is in the form of a capsule. 